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An ideal gas, Cv=5/2R is expanded adiabatically against a constant pressure of 1atm untill it doubles in volume.If the initial temperature is 25degree celsius and the initial pressure is 5atm,the value of T2 is?
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An ideal gas, Cv=5/2R is expanded adiabatically against a constant pre...
Given


  • Cv = 5/2R

  • Adiabatic expansion

  • Constant pressure = 1 atm

  • Volume doubles

  • Initial temperature = 25°C = 298K

  • Initial pressure = 5 atm



Solution

Step 1: Finding initial volume and moles of gas

Using ideal gas equation, PV = nRT

Initial volume, V1 = nRT1/P1 = (1 mole x 5 atm x 298K) / 5 atm = 298 L

Number of moles, n = PV/RT = (5 atm x 298 L) / (0.082 L atm/K mol x 298 K) = 1.82 moles


Step 2: Finding final temperature and volume

Using adiabatic expansion equation, P1V1^γ = P2V2^γ where γ = Cp/Cv = 7/5 for ideal gas

Final volume, V2 = 2 x V1 = 596 L

Final pressure, P2 = P1(V1/V2)^γ = 5(1/2)^7/5 = 2.07 atm

Using ideal gas equation, P2V2 = nRT2

Final temperature, T2 = P2V2/nR = (2.07 atm x 596 L) / (1.82 mol x 0.082 L atm/K mol) = 638K


Answer

The final temperature, T2 = 638K.
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An ideal gas, Cv=5/2R is expanded adiabatically against a constant pressure of 1atm untill it doubles in volume.If the initial temperature is 25degree celsius and the initial pressure is 5atm,the value of T2 is?
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